Bases Arrhenius concept

There are certain limitations of the Arrhenius concept of acids and bases. Acids and bases have been described in terms of their aqueous solutions and not in terms of the entities themselves. The theory is thus applicable exclusively to aqueous solutions. An entity such as HC1 is accounted as an acid only when it is dissolved in water if dissolved in... 

Any text on acids and bases would not be deemed complete if mention were not made of the extended definition of acids and bases that is embodied in the Lowry-Bronsted theory. The theory basically proposed a more general definition of acids and bases to overpower the limitations of the theory arising from the Arrhenius concept. 

The Arrhenius concept was of basic importance because it permitted quantitative treatment of a number of acid-base processes in aqueous solutions, i.e. the behaviour of acids, bases, their salts and mixtures of these substances in aqueous solutions. Nonetheless, when more experimental material was collected, particularly on reaction rates of acid-base catalysed processes, an increasing number of facts was found that was not clearly interpretable on the basis of the Arrhenius theory (e.g. in anhydrous acetone NH3 reacts with acids in the absence of OH- and without the formation of water). It gradually became clear that a more general theory was needed. Such a theory was developed in 1923 by J. N. Br0nsted and, independently, by T. M. Lowry. 

Acid-base reactions concepts of Arrhenius, Brpnstcd-Lowry, and Lewis coordination complexes, amphoterism... 

Each of the three definitions expands our concept of acids and bases. Arrhenius basic definition is adequate for understanding many of the properties of acids and bases. It is important to recognize, though, that acids and bases are not fixed labels that can be applied to a substance. Bronsted-Lowry and Lewis showed that acid-base characteristics are dependent on the reactions that take place between substances. A... 

Arrhenius concept A concept stating that acids produce hydrogen ions and bases produce hydroxide ions in aqueous solutions. 

Note that HA and B are not necessarily neutral. They could be ions that are capable of acting as an acid or a base. This is one of the features of the Bronsted-Lowry concept that broadens the definitions of acids and bases over the Arrhenius concept—there are many more substances that can behave as acids or bases. Further, we can write the reaction including the solvent, water in this case, and the associated Ka. 

The first person to recognize the essential nature of acids and bases was Svante Arrhenius. Based on his experiments with electrolytes, Arrhenius postulated that acids produce hydrogen ions in aqueous solution, and bases produce hydroxide ions. At the time of its discovery the Arrhenius concept of acids and bases was a major step forward in quantifying acid—base chemistry, but this concept is limited because it applies only to aqueous solutions and allows for only one kind of base—the hydroxide ion. A more general definition of acids and bases was suggested independently by the Danish chemist Johannes N. Bronsted (1879-1947) and the English chemist Thomas M. Lowry (1874-1936) in 1923. In terms of the Bronsted—Lowry definition, an acid is a proton (H+) donor, and a base is a proton acceptor. For example, when gaseous HCl dissolves in water, each HCl molecule donates a proton to a water molecule, and so HCl qualifies as a Bronsted-Lowry acid. The molecule that accepts the proton—water in this case—is a Bronsted-Lowry base. 

Note that this reaction is not considered an acid-base reaction according to the Arrhenius concept. 

According to the Arrhenius concept, a base is a substance that produces OH-ions in aqueous solution. According to the Bronsted-Lowry definition, a base is a proton acceptor. The bases sodium hydroxide (NaOH) and potassium hydroxide (KOH) fulfill both criteria. They contain OH- ions in the solid lattice and behave as strong electrolytes, dissociating completely when dissolving in water ... 

Aromatic hydrocarbon one of a special class of cyclic unsaturated hydrocarbons, the simplest of which is benzene. (22.3) Arrhenius concept a concept postulating that acids produce hydrogen ions in aqueous solution, whereas bases produce hydroxide ions. (7.1)... 

Arrhenius Concept Arrhenius (1887) defined acid as a substance that will dissociate to yield a hydrogen ion while base in one that will dissociate to yield a hydroxyl ion in aqueous solution. 

Regarding the question, what do you understand by the term acid or base , many students respond with a pH value ( acids have a small pH value ) or with simple, but misconceived phenomena, which are formulated as follows Adds eat away, are dangerous, yellow, red or acidic [4], Other statements describe acid concepts, which have been mainly learned and remembered Approximately 15% of the answers show the Arrhenius concept (acids contain H + ions) approximately 30% show the Broensted concept (acids release protons), whereby it is not certain if students correctly understand the notion of acids as acid particles. 

Acid-Base Concepts. In the lesson, after becoming familiar with many phenomena on acids and bases as substances, the question is raised as to whether the substance-related Arrhenius concept should be taught, or the particle-related Broensted concept - or the genetic development of both concepts in the form of historically oriented lessons (see Fig. 7.2). Tests on electrical conductivity of solutions of strong acids and bases (see E7.7) confirms that acidic solutions contain H + (aq) ions and basic solutions contain OH (aq) ions. After stating the existence of these ions, one can discuss model drawings and emphasize that the (aq) symbol denotes the complete separation of the ions by hydration (see Figs. 7.10 and 7.11). 

Mental models are thus produced of both acid concepts those of Arrhenius and of Broensted. The Arrhenius concept explains some phenomena in the area of acids and bases, for instance, the neutralization of solutions of strong acids and bases. Terms like weak acids or derived concepts like acid constants or buffer already reach the limits of Arrhenius concept. 

If you missed 43, go to The Arrhenius Concept of Acids and Bases, page 394. 

The Arrhenius concept of acids and bases was a tremendous advance in the understanding of these compounds, but is it limited to aqueous solutions, and a lot of chemistry takes place out of water. In 1923 a Danish chemist, Johannes Bronsted (1879-1947), and an English chemist, Thomas Lowry (1874-1936), proposed a more general way to describe acids and bases centered on the ability of a species to donate or accept a proton, IT. It was not limited to aqueous solutions. Here is how they defined acids, bases and neutralization ... 

The Bronsted-Lowry concept describes many more processes as acid-base reactions than does the Arrhenius concept. For example, the ionization of hydrogen chloride gas as it dissolves in water, HC1 (g) — HC1 (aq), can be described as an acid-base process as the proton from HC1 is transferred to water. 

All compounds that are acids and bases in the Arrhenius concept are also acids and bases in the Bronsted-Lowry scheme. Ammonia gas, NH3fgJ, is very soluble in water, quickly engaging in an equilibrium that produces hydroxide ion making the solution basic. In doing so, water acts as a Bronsted-Lowry acid, donating a proton to ammonia, leaving the remainder of the water molecule, the hydroxide ion, behind. 

In the Arrhenius concept of acids and bases, what species are produced by acids and bases in water What is formed from these species in neutralization ... 

When ammonia is dissolved in water, it can accept a proton from water to form the ammonium ion, and hydroxide ion. Ammonia is a base in the Arrhenius concept because it produces hydroxide ion in water, and it is a base in the Bronsted-Lowiy concept because it is a proton acceptor. 

Arrhenius concept (14) An acid-base concept in which an acid produces hydrogen ion (hydronium ion) and a base produces hydroxide ion when dissolved in water. Neutralization combines hydronium and hydroxide ions to form water. 

Although the Arrhenius concept of acids and bases was a major step forward in understanding acid-base chemistry, this concept is limited because it allows for only one kind of base—the hydroxide ion. A more general definition of acids and bases was suggested by the Danish chemist Johannes Bronsted and the English chemist Thomas Lowry. 

Arrhenius concept Bronsted-Lowry model hydronium ion conjugate base conjugate acid conjugate acid-base pair acid dissociation constant Section 14.2 strong acid weak acid diprotic acid oxyacids organic acids carboxyl group monoprotic acids amphoteric substance autoionization... 

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